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VITEEE Chemistry Syllabus 2023 : VIT Engineering Entrance Exam

Organisation : Vellore Institute of Technology
Exam Name : VIT Engineering Entrance Examination VITEEE
Service Name : VITEEE 2023 Syllabus
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Vellore Institute of Technology Engineering Entrance Examination (VITEEE) is conducted for admission to undergraduate engineering programmes in VIT group of Institutions. VITEEE will be conducted between 15 and 21 April 2023 (Tentative) at designated centres across India and abroad. VITEEE is a common entrance exam for VIT Vellore, VIT Chennai, VIT-AP and VIT- Bhopal.

Related / Similar Syllabus : GATE Instrumentation Engineering (IN) Syllabus 2023

VITEEE Chemistry Syllabus

Physical Chemistry
** Atomic Structure – Bohr’s atomic model-Sommerfeld’s extension of atomic structure; Electronic configuration and Quantum numbers; Shapes of s, p, d, f orbitals – Pauli’s exclusion principle – Hund’s Rule of maximum multiplicity- Aufbau principle. Emission and absorption spectra, line and band spectra; Hydrogen spectrum – Lyman, Balmer, Paschen, Brackett and Pfund series; de Broglie’s theory; Heisenberg’s uncertainty principle – wave nature of electron– Schrodinger wave equation (No derivation). Eigen values and eigen functions.

** Chemical bonding and hybridization of atomic orbitals involving s, p and d orbitals. Thermodynamics, Chemical Equilibrium and Chemical Kinetics – I and II Laws of thermodynamics – spontaneous and non-spontaneous processes, entropy, Gibb’s free energy – Standard Gibbs free energy change (ΔG0) and chemical equilibrium – significance of entropy. Rate of a chemical reaction, factors affecting rates of reaction: concentration, temperature, pressure and catalyst; Law of mass action – Le Chatelier’s principle, applications of chemical equilibrium. Rate expression, order, and molecularity of reactions, zero order, first order and pseudo first order reaction – half-life period.

** Determination of rate constant and order of reaction. Temperature dependence of rate constant – Arrhenius equation, activation energy and its calculation; elementary concept of collision theory of bimolecular gaseous reactions. Solutions – Colligative properties of dilute solutions; Different methods for expressing the concentration of solution – molality, molarity, mole fraction, percentage, the vapour pressure of solutions and Raoult’s Law – Ideal and non-ideal solutions, vapour pressure – composition, plots for ideal and non-ideal solutions

2. Inorganic and Material Chemistry
** The s-block elements – properties and chemical reactivity of alkali and alkaline earth metals The p-block elements – Phosphorous compounds: PCl3, PCl5 – Oxides, Hydrogen halides, Inter-halogen compounds and Xenon fluoride compounds General characteristics of d – block elements – Electronic Configuration – Oxidation states of first row transition elements and their colours. Occurrence and principles of extraction: Copper, Silver, Gold and Zinc. Preparation and properties of CuSO4, AgNO3 and K2Cr2O7. Lanthanides – Introduction, electronic configuration, general characteristics, oxidation state – lanthanide contraction, uses, brief comparison of Lanthanides and Actinides Introduction to coordination chemistry – IUPAC nomenclature of mononuclear coordination compounds; Isomerism, Geometrical isomerism in 4-coordinate, 6-coordinate complexes.

** Theories on coordination compounds – Werner’s theory (brief), Valence Bond theory. Uses of coordination compounds. Bioinorganic compounds (Haemoglobin and chlorophyll). Solid-State Chemistry – Lattice – unit cell, systems, types of crystals, packing in solids; Ionic crystals – Imperfections in solids – point defects, X-Ray diffraction – Electrical Property, Amorphous solids (elementary ideas only) Surface Chemistry – Adsorption- physisorption and chemisorption; Catalysis – homogeneous and heterogeneous catalysis

3. Analytical Chemistry
Electrochemistry – Redox reactions; Theory of electrical conductance; metallic and electrolytic conductance. Faraday’s laws – theory of strong electrolytes – Specific resistance, specific conductance, equivalent and molar conductance – Variation of conductance with dilution – Kohlrausch’s Law – Ionic product of water, pH, and pH– buffer solutions – use of pH values. Cells – Electrodes and electrode potentials – construction of cell, EMF values and standard electrode potentials, Nernst equation and its application to chemical cells. Relation between Gibbs energy change and EMF of a cell, dry cell, electrolytic cells and Galvanic cells; lead accumulator; Fuel cells, Corrosion, and its prevention. Environmental Chemistry – Environmental pollution – Atmospheric, water and soil.

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